Question

(9) Potassium chlorate decomposes when heated to produce potassium chloride and oxygen gas: 2 KClO? (s) ? 2 KCl (s) + 3 O? (g) (a) If a test tube holding 87 g KClO? is heated and the reaction goes to completion, calculate the volume of O? gas that will be obtained if it is collected at a pressure of 1 atm and temperature of 27 °C. (Assume ideal gas behavior.) (b) If the same reaction is instead performed in a closed vessel of 2.0 L at 27 °C, calculate the pressure at reaction completion using the ideal gas law. (c) Now calculate the pressure at reaction completion in a closed vessel of 2.0 L at 27 °C using the Van der Waals equation (a=1.36 atm L² mol?², b=0.03186 L mol?¹) (d) In general (not just this problem), which experimental conditions cause the greatest disparity between results obtained from the ideal gas equation versus the Van der Waals equation.

          (9) Potassium chlorate decomposes when heated to produce potassium chloride and oxygen gas: 2 KClO? (s) ? 2 KCl (s) + 3 O? (g) (a) If a test tube holding 87 g KClO? is heated and the reaction goes to completion, calculate the volume of O? gas that will be obtained if it is collected at a pressure of 1 atm and temperature of 27 °C. (Assume ideal gas behavior.) (b) If the same reaction is instead performed in a closed vessel of 2.0 L at 27 °C, calculate the pressure at reaction completion using the ideal gas law. (c) Now calculate the pressure at reaction completion in a closed vessel of 2.0 L at 27 °C using the Van der Waals equation (a=1.36 atm L² mol?², b=0.03186 L mol?¹) (d) In general (not just this problem), which experimental conditions cause the greatest disparity between results obtained from the ideal gas equation versus the Van der Waals equation.

(9) Potassium chlorate decomposes when heated to produce potassium chloride and oxygen gas: 2 KClO? (s) ? 2 KCl (s) + 3 O? (g) (a) If a test tube holding 87 g KClO? is heated and the reaction goes to completion, calculate the volume of O? gas that will be obtained if it is collected at a pressure of 1 atm and temperature of 27 °C. (Assume ideal gas behavior.) (b) If the same reaction is instead performed in a closed vessel of 2.0 L at 27 °C, calculate the pressure at reaction completion using the ideal gas law. (c) Now calculate the pressure at reaction completion in a closed vessel of 2.0 L at 27 °C using the Van der Waals equation (a=1.36 atm L² mol?², b=0.03186 L mol?¹) (d) In general (not just this problem), which experimental conditions cause the greatest disparity between results obtained from the ideal gas equation versus the Van der Waals equation.

Added by Joseph R.

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